AP Chemistry Summer Assignment 2018-2019

1 AP Chemistry Summer Assignment 2018-2019 The AP Chemistry Summer Assignment is completely online! We will be using an online program called Mastering Chemistry . Once you are enrolled in the online course (via blackboard), you will be responsible for completing the 5 part Summer Assignment . You must have a correct email address in blackboard. Information on how to login to the website will be emailed to you. Go under the My FCPS tab and click on personal information in the tools section if you need to edit your email address on blackboard. 1. Summer Assignment Part 1 Introduction to MasteringChemistry This is an optional Assignment . This will allow you to get familiar with the online program. 2. Summer Assignment Part 2 Chapter 01 Practice Problems Note that the tutorials are not worth any points. These are optional if you need to learn the items again.

2 You SHOULD be able to answer all problems based on your knowledge from your first year of tutorials will help you get familiar with everything. You will have 6 opportunities to complete all mandatory questions correctly before you cannot receive credit. You may use hints and you will not be penalized! 3. Summer Assignment Part 3 Chapter 02 Practice Problems Same guidelines as part 2 4. Summer Assignment Part 4 Chapter 03 Practice Problems Same guidelines as part 2 5. Summer Assignment Part 5 Multiple Choice Test (Chapters 1 3 ) Once you complete parts 2, 3 and 4 you will take this test. The test is 50 questions multiple choice. You are allowed 2 attempts to get the correct answer before you lose credit. No hints 6. Additional Packet a. Please commit to memory the pages that say MEMORIZE this (multiple oxidation metals, polyatomic ions, strong acids/bases, and solubility rules).

3 B. Look over the reactions and color guide. Since there are many reactions and we will be learning reactions in the first unit, it is in your best interest to have a solid grasp from day one! 7. Textbook a. This year in AP Chemistry we will be using Chemistry : The Central Science Twelfth Edition, AP Edition. By Brown, LeMay, Bursten, Murphy, Woodward. b. You will have online access to this textbook through the MasteringChemistry course. c. You can pick up a hard copy of the text from Ms. Saccomando in Room 301 or Ms. Malik starting on June 15th (please note that a hard copy is not necessary to have to complete the Summer Assignment ). If you have any questions, please email Ms. Saccomando at or Ms. Malik at . Ionic Compounds (MEMORIZE THIS PAGE!) Common Metal Ions with More than One Ionic Charge (MOM) Symbol Stock Name Classical Name Cu+ Copper(I) ion Cuprous ion Cu2+ Copper(II) ion Cupric ion Fe2+ Iron(II) ion Ferrous ion Fe3+ Iron (III) ion Ferric ion Hg2+ Mercury(II) ion Mercuric ion Pb2+ Lead(II) ion Plumbous ion Pb4+ Lead(IV) ion Plumbic ion Sn2+ Tin(II) ion Stannous ion Sn4+ Tin(IV) ion Stannic ion Cr2+ Chromium(II) ion Chromous ion Cr3+ Chromium(III) ion Chromic ion Mn2+ Manganese(II) ion Manganous ion Mn3+ Manganese(III) ion Manganic ion Co2+ Cobalt(II) ion Cobaltous ion Co3+ Cobalt(III) ion Cobaltic ion **Note Silver ion and Zinc ion and Cadmium ion are all transition metal ions, but they only have 1 charge (1 oxidation state) so they do NOT need a roman numeral.

4 (Ag+ and Zn2+ and Cd2+) Common Polyatomic Ions Name Formula Name Formula Ammonium NH4+ Iodate IO3- Nitrite NO2- Periodate IO4- Nitrate NO3- Acetate C2H3O2- Hydrogen Sulfate HSO4- Dihydrogen Phosphate H2PO4- Hydroxide OH- Carbonate CO32- Cyanide CN- Sulfite SO32- Permanganate MnO4- Sulfate SO42- Hydrogen Carbonate HCO3- Thiosulfate S2O32- Hypochlorite ClO- Peroxide O22- Chlorite ClO2- Chromate CrO42- Chlorate ClO3- Dichromate Cr2O72- Perchlorate ClO4- Hydrogen Phosphate HPO42- Bromate BrO3- Phosphite PO33- Hydronium H3O+ Phosphate PO43- The old way to say hydrogen carbonate was bicarbonate ..if you see the prefix bi in front of a polyatomic ion name, then you are adding an H+ to the that when you add an H+ to the formula the net charge of the ion goes down = = HCO31- Bisulfate = HSO4- MEMORIZE this page as well TABLE OF STRONG ACIDS TABLE OF STRONG BASES Completely Ionized in Water to Give One (or more) Protons Complete ionize to give one (or more) Hydroxides HI H+(aq) + I-(aq) HBr H+(aq) + Br-(aq) HClO4 H+(aq) + ClO4-(aq) HCl H+(aq) + Cl-(aq) HClO3 H+(aq) + ClO3-(aq) H2SO4 H+(aq) + HSO4-(aq) (HSO4- is a weak acid) HNO3 H+(aq) + NO3-(aq) SOLUBILITY RULES: 1.

5 Alkali metal salts AND NH4+ salts ARE soluble 2. NO3-, ClO3-, ClO4-, and CH3 COO- are soluble 3. Cl-, Br-, I- are soluble, *except for Ag+, Hg2+2, Pb+2 3. F- are soluble, *except for Group II metals 4. SO4-2 are soluble, *except for Ca2+, Sr+2, Ba+2, Ag+, Pb+2, Hg22+ 5. CO3-2, PO4-3, C2O4-2, CrO4-2, S-2, OH-, and O-2 are INSOLUBLE **unless it is group I (rule 1 takes priority!)** It can be assumed that ionic compounds that dissolve in water are strong electrolytes and are therefore soluble. NaOH Na+(aq) + OH-(aq) KOH K+(aq) + OH-(aq) LiOH Li+(aq) + OH-(aq) RbOH Rb+(aq) + OH-(aq) CsOH Cs+(aq) + OH-(aq) Ca(OH)2 Ca2+(aq) + 2OH-(aq) Ba(OH)2 Ba2+(aq) + 2OH-(aq) Sr(OH)2 Sr2+(aq) + 2OH-(aq) AP Chemistry Predicting the Products Rules & Tidbits to remember (This is what we will be learning in ) Synthesis reactions A + B AB 1.

6 A metal combines with a nonmetal to for a binary salt (IONIC COMPOUND) Ex. A piece of magnesium ribbon is placed in a container with oxygen gas. Equation: 2Mg(s) + O2(g) 2 MgO(s) Net Ionic: 2Mg(s) + O2(g) 2 MgO(s)..*Note that there is no water so the ionic compound will not be aqueous, so it will not be dissociated!!!! 2. Metallic Oxides (Ionic compounds with oxygen as the anion) added to water will form bases (Ionic compounds with Hydroxide as the anion) Ex. Solid barium oxide is added to water. Equation: BaO(s) + H2O(l) Ba(OH)2(aq) *Note that the compound was added to water so the product is aqueous Net Ionic: BaO(s) + H2O(l) Ba2+ + 2OH- *Note that barium hydroxide is a strong base so it will be written dissociated in the net ionic equation! 3. Nonmetallic oxides (Covalent Compounds with oxygen) added to water will form acids.

7 The nonmetal attached to oxygen in the nonmetallic oxide will keep its oxidation number. Ex. Carbon dioxide is bubbled through water. Equation: CO2(g) + H2O(l) H2CO3(aq) *Note that the oxidation number for carbon is still +4, and that Carbonic acid is aqueous because it is in water. Net Ionic: CO2(g) + H2O(l) H2CO3(aq) *Note that carbonic acid is NOT dissociated because it is a WEAK acid 4. Metallic oxides combined with nonmetallic oxides will for Ionic compounds with polyatomic ions Ex. Crystals of sodium oxide are added to a container with sulfur dioxide gas. Equation: Na2O(s) + SO2(g) Na2SO3(s) *Note that the sulfur maintains its oxidation is why the product is not Na2SO4. Also note that the product is a solid because there is no it CANNOT BE AQUEOUS! Net Ionic: Na2O(s) + SO2(g) Na2SO3(s) *Note that nothing dissociates when there is no aqueous species Decomposition Reactions AB A + B (compounds generally start out as a solid) 1.

8 Metallic Carbonates (Ionic compounds with carbonate) decompose into metallic oxides and carbon dioxide. Ex. Potassium carbonate is heated Equation: K2CO3(s) K2O(s) + CO2(g) Net Ionic: K2CO3(s) K2O(s) + CO2(g) *No dissociation! 2. Metallic Chlorates (Ionic compounds with chlorate) decompose into metallic chlorides and oxygen Ex. A sample of magnesium chlorate is heated. Equation: Mg(ClO3)2(s) MgCl2(g) + 3O2(g) Net Ionic: Mg(ClO3)2(s) MgCl2(g) + 3O2(g) *No dissociation! 3. Ammonium Carbonate decomposes into ammonia, water and carbon dioxide. Ex. A sample of ammonium carbonate is heated Equation: (NH4)2CO3(s) 2NH3(g) + H2O(l) + CO2(g) Net Ionic: (NH4)2CO3(s) 2NH3(g) + H2O(l) + CO2(g) *Note that gases never dissociate so nothing will be written dissociated! 4. Sulfurous acid decomposes into sulfur dioxide and water Ex.

9 A sample of sulfurous acid is heated. Equation: H2SO3(aq) H2O(l) + SO2(g) *Note that sulfurous acid is aqueous because it is an acid Net Ionic: H2SO3(aq) H2O(l) + SO2(g) *Note that sulfurous acid does not dissociate because it is a weak acid! 5. Carbonic acid decomposes into carbon dioxide and water. Ex. A solution of carbonic acid is heated Equation: H2CO3(aq) H2O(l) + CO2(g) *Note carbonic acid is aqueous because it is an acid Net Ionic: H2CO3(aq) H2O(l) + CO2(g) *Note that carbonic acid does not dissociate because it is a weak acid! 6. A binary compound (Ionic compounds made of monatomic ions) may break down to produce two starts with a molten (liquid) ionic compound being electrolyzed Ex. Molten aluminum chloride is electrolyzed. Equation: 2 AlCl3(l) 2Al(s) + 3Cl2(g) *Note this will be the only time you have a liquid ionic compound Net Ionic: 2 AlCl3(l) 2Al(s) + 3Cl2(g) 7.

10 Hydrogen peroxide decomposes into water and oxygen. Ex. A sample of hydrogen peroxide is heated Equation: 2H2O2(aq) 2H2O(l) + O2(g) *Note hydrogen peroxide will always be in solution so it will be aqueous Net Ionic: 2H2O2(aq) 2H2O(l) + O2(g) *Hydrogen peroxide does NOT dissociate 8. Ammonium Hydroxide decomposes into ammonia and water Ex. Ammonium hydroxide is heated. Equation: NH4OH(aq) NH3(g) + H2O(l) *Note that ammonia hydroxide is always in an aqueous solution Net Ionic: NH4OH(aq) NH3(g) + H2O(l) *Note that ammonia hydroxide does not dissociate because it acts as weak conjugate acid! Single Replacement Reactions (A + BC B + AC) 1. Active metals will replace less active metals from their compounds in an aqueous solution. Ex. Calcium deposits are added to a solution of Iron (III) chloride Equation: 3Ca(s) + 2 FeCl3(aq) 2Fe(s) + 3 MgCl2(aq) Net Ionic: 3Ca(s) + 2Fe3+ 2Fe(s) + 3Mg2+ *Note that the metal that gets replaced is now in its normal elemental form with oxidation state of zero 2.